Suppose you are a food chemist working for a company that makes and manufactures soda. your job is to create a new soft drink with the ingredients available to you. there is one problem—you need 1 liter of phosphoric acid solution, and the phosphoric acid available to use has a concentration of 0.01 m. this is much too high to add to your soda without distorting the flavor. typically, there are about 45 milligrams of phosphoric acid per 12 ounce can of soda. here is your task:

convert the 45 milligrams of phosphoric acid (h3po4) into grams and then into moles.
0.00046 moles or 4.6×10-4 moles
given that 12 ounces is equal to about 0.35 liter, find the molarity of the phosphoric acid in a typical can of soda (45 milligrams). 0.0013 m or 1.3×10-3 m
using the dilution equation, determine how much of the stock solution (0.01 m h3po4) you will need to make 1 liter of the concentration typically used in soda.
0.13 liter or 130 milliliters

The answer to your question is given after the questions so I just explain how to get it.

Explanation:

a)

Get the molecular weight of Phosphoric acid

        H₃PO₄ =  (3 x 1) + (31 x 1) + (16 x 4)

                    = 3 + 31 + 64

                    = 98 g

         98 g -----------------  1 mol

      0.045 g ---------------   x

          x = (0.045 x 1) / 98

          x = 0.045 / 98

          x = 0.00046 moles or 4.6 x 10 ⁻⁴

b)

Molarity =

Molarity =

Molarity = 0.0013 or 1.31 x 10⁻³

c)

Formula            C₁V₁ = C₂V₂

                              V₁ = C₂V₂ / C₁

Substitution

                              V₁ = (0.0013)(1) / 0.01

Simplification and result

                              V₁ = 0.0013 / 0.1

                              V₁ = 0.13 l = 130 ml            

45 mg × 1 g/1000 mg = 0.045 g

0.045 g × 1 mol/98 g = 0.00046 mol

0.00046 mol/0.35 L = 0.0013 M

0.01 M × x = 0.0013 M × 1 L

Solution: 130 milliliter

Answer from Edmentum

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

c is the answer because when something is left after something evaporates that shows the chemical change.